Concept explainers
(a)
Interpretation:
All resonance contributors for sulfuric acid
Concept introduction:
If a species having two or more valid Lewis structures, then its resonance structure exists. Resonance structures are imaginary; true species is represented by the resonance hybrid. The resonance structures are differed by the placement of their valence electrons, and not their atoms. Resonance structures with a greater number of atoms having an octet complete, more covalent bonds, and fewer atoms having a non-zero formal charge are considered to be stable. While drawing resonance structures curved arrows are used. The movement of a pair of electrons is indicated by a curved arrow. A curved arrow originates from a lone pair of electrons or from a covalent double or triple bond to indicate the specific pair of electrons that are being moved. The arrow points to an atom if the electrons being moved become a lone pair. Otherwise, the arrow points to the center of an existing bond to represent the formation of a new double/triple bond. A resonance structure can be drawn if a lone pair of electrons on an atom is adjacent with multiple bonds or an incomplete octet on an atom is adjacent to multiple bonds or there is a ring of alternating single and multiple bonds.
(b)
Interpretation:
Resonance hybrid for
Concept introduction:
A resonance hybrid structure is a weighted average structure of all the resonance contributors. A partial bond is represented in a resonance hybrid by a dashed line connecting the two atoms. In the resonance hybrid, the partial bonds are shown, which represent the atoms over which the electrons are delocalized. The resonance hybrid structure looks most like the lowest energy resonance structure and it is the most stable structure. The more stable resonance structures have a) a greater number of atoms having octet complete, b) more number of covalent bonds, and c) fewer atoms having a non-zero formal charge.
(c)
Interpretation:
The resonance structures of
Concept introduction:
A resonance hybrid structure is a weighted average structure of all the resonance contributors. A partial bond is represented in a resonance hybrid by a dashed line connecting the two atoms. In the resonance hybrid, the partial bonds are shown, which represent the atoms over which the electrons are delocalized. The resonance hybrid structure looks most like the lowest energy resonance structure and it is the most stable structure. The more stable resonance structures have a) a greater number of atoms having octet complete, b) more number of covalent bonds, and c) fewer atoms having a non-zero formal charge.
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- Calculate the enthalpy change for the following reactions using the bond enthalpy given below. (Bond enthalpy/kJ : H−H = 436, C−H = 413, C=O = 799, O=O = 495, O−H = 463) (a) H2(g) + 1⁄2O2(g) → H2O(g) (b) CH4(g) + 2O2(g) → CO2(g) + 2H2O(l)arrow_forward(a) Determine the formal charge of oxygen in the following structure. If the atom is formally neutral, indicate a charge of zero. (b) Draw an alternative Lewis (resonance) structure for the compound given in part (a). Show the unshared pairs and nonzero formal charges in your structure. Don't use radicals. Formal charge on O 0arrow_forwardWhich statements are true about resonance contributing structures? (a) All contributing structures must have the same number of valence electrons. (b) All contributing structures must have the same arrangement of atoms. (c) All atoms in a contributing structure must have complete valence shells. (d) All bond angles in sets of contributing structures must be the same.arrow_forward
- Draw Lewis structures and any contributing resonance structures for each structure below. Use the proper type of arrow to indicate that they are resonance structures. In which structure is resonance more important? (a) H2SO3 (b) (HSO3)^1- (c) (SO3)^2-arrow_forwardHydrazine, N₂H₄, and carbon disulfide, CS₂, form a cyclicmolecule(right).(a) Draw Lewisstructures for N₂H₄ and CS₂. (b) How do electron-group arrange-ment, molecular shape, and hy-bridization of N change when N₂H₄ reacts to form the product?(c) How do electron-group arrangement, molecular shape, andhybridization of C change when CS₂ reacts to form the product?arrow_forwardIn addition to ammonia, nitrogen forms three other hy-drides: hydrazine (N₂H₄), diazene (N₂H₂), and tetrazene (N₄H₄).(a) Use Lewis structures to compare the strength, length, and or-der of nitrogen-nitrogen bonds in hydrazine, diazene, and N₂.(b) Tetrazene (atom sequence H₂NNNNH₂) decomposes above 0°C to hydrazine and nitrogen gas. Draw a Lewis structure fortetrazene, and calculate ΔH°ᵣₓₙ for this decomposition.arrow_forward
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- Draw a Lewis structure for each of the following molecules: (a) chlorodifluoromethane, CHClF2 (b) propanoic acid, C2 H5CO2H (basic structure pictured below) (c) acetonitrile, CH3CH (the framework is H3C-C-N) (d) allene, H3CCCH2arrow_forwardThe two compounds nitrogen dioxide and dinitrogen tetraoxide are introduced in Section 3.13. (a) NO2 is an odd-electron compound. Draw the best Lewis diagrams possible for it, recognizing that one atom cannot achieve an octet configuration. Use formal charges to decide whether that should be the (central) nitrogen atom or one of the oxygen atoms. (b) Draw resonance forms for N2O4 that obey the octet rule. The two N atoms are bonded in this molecule.arrow_forwardDraw all possible resonance structures for each of these compounds. Determine the formal charge on each atom in each of the resonance structures:(a) O3(b) SO2(c) NO2 −(d) NO3−arrow_forward
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning